The measured osmotic pressure of a solution prepared by dissolving 17.4 mg of K2SO4 in 2L of water at 27 °C is 3.735 × 10-3 bar. The Van' t Hoff factor is (R = 0.083 L bar K-1 mol-1: atomic weights K = 39: S = 32: O = 16)

Question

The measured osmotic pressure of a solution prepared by dissolving 17.4 mg of K2SO4 in 2L of water at 27 °C is 3.735 × 10-3 bar. The Van' t Hoff factor is (R = 0.083 L bar K-1 mol-1: atomic weights K = 39: S = 32: O = 16) (A) 2.84 (B) 3.0 (C) 2.0 (D) 2.32

Tardigrade Admin · Accepted Answer

Given, π=3.735 × 10-3 bar Mass of K 2 SO 4(ω)=17.4 mg Volume =2 L Temperature (T)=27° C =27+273=300 K From osmotic pressure of solution. π =i C R T i = van't-Hoff factor i =π / C R T =(π × M × V/ω × R × T)=(3.735 × 174 × 2/17.4 × 0.083 × 300) Molar mass (M) H 2 SO 4=174, i=3.0

Q. The measured osmotic pressure of a solution prepared by dissolving 17.4mg of K2​SO4​ in 2L of water at 27∘C is 3.735×10−3 bar. The Van' t Hoff factor is (R=0.083L bar K−1mol−1 : atomic weights K=39:S=32:O=16)

2.84

3.0

2.0

2.32

Given, π=3.735×10−3 bar Mass of K2​SO4​(ω)=17.4mg Volume =2L Temperature (T)=27∘C=27+273=300K From osmotic pressure of solution. π=iCRT i= van't-Hoff factor i=π/CRT =ω×R×Tπ×M×V​=17.4×0.083×3003.735×174×2​ Molar mass (M)H2​SO4​=174,i=3.0

Q. The measured osmotic pressure of a solution prepared by dissolving $17.4 m g$ of $K_{2} S O_{4}$ in $2 L$ of water at $27^{\circ} C$ is $3.735 \times 1 0^{- 3}$ bar. The Van' t Hoff factor is
( $R = 0.083 L$ bar $K^{- 1} m o l^{- 1}$ : atomic weights $K = 39 : S = 32 : O = 16$ )